Skip to main content
Ch.3 - Mass Relationships in Chemical Reactions

Chapter 3, Problem 117b

A copper wire having a mass of 2.196 g was allowed to react with an excess of sulfur. The excess sulfur was then burned, yielding SO2 gas. The mass of the copper sulfide produced was 2.748 g. (b) What is its empirical formula?

Verified Solution
Video duration:
1m
This video solution was recommended by our tutors as helpful for the problem above.
550
views
Was this helpful?

Video transcript

Hey everyone, welcome back. We're asked to provide the empirical formula for a substance consisting of 1.78g of copper and 2.22g of selenium first. Let's go ahead and convert our grams into moles. Starting off with 1.78 g of copper. We're going to use coppers atomic mass of 63. g per one mole. And when we calculate this out, we end up with a value of 0. mol of copper. Moving on to selenium, we have 2.22g of selenium And we know that selenium is atomic mass is 78.96 g of selenium per one mole. And when we calculate this out, we end up with a total of 0.02, a mole of selenium. And now all we need to do is divide both of our values by the least amount of moles. And in this case since both of our values are 0.028, All we need to do is divide them both by 0.028 which gets us to one of copper and one of selenium. So our empirical formula is going to be C U S E. So I hope this made sense and let us know if you have any questions
Related Practice
Textbook Question

A compound of formula XCl3 reacts with aqueous AgNO3 to yield solid AgCl according to the following equation: When a solution containing 0.634 g of XCl3 was allowed to react with an excess of aqueous AgNO3, 1.68 g of solid AgCl was formed. What is the identity of the atom X?

336
views
Textbook Question
When eaten, dietary carbohydrates are digested to yield glu-cose (C6H12O6), which is then metabolized to yield carbon dioxide and water: Balance the equation, and calculate both the mass in grams and the volume in liters of the CO2 produced from 66.3 g of glucose, assuming that 1 mol of CO2 has a volume of 25.4 L at normal body temperature.
524
views
Textbook Question

A copper wire having a mass of 2.196 g was allowed to react with an excess of sulfur. The excess sulfur was then burned, yielding SO2 gas. The mass of the copper sulfide produced was 2.748 g. (a) What is the percent composition of copper sulfide?

604
views
Textbook Question
Element X, a member of group 5A, forms two chlorides, XCl3 and XCl5. Reaction of an excess of Cl2 with 8.729 g of XCl3 yields 13.233 g of XCl5. What is the atomic weight and the identity of the element X?
628
views
Textbook Question

Ammonium nitrate, a potential ingredient of terrorist bombs, can be made nonexplosive by addition of diammo-nium hydrogen phosphate, (NH4)2HPO4. Analysis of such a NH4NO3 - (NH4)2HPO4 mixture showed the mass percent of nitrogen to be 30.43%. What is the mass ratio of the two components in the mixture?

720
views
Textbook Question
Window glass is typically made by mixing soda ash (Na2CO3), limestone (CaCO3), and silica sand (SiO2) and then heating to 1500 °C to drive off CO2 from the (Na2CO3) and CaCO3. The resultant glass consists of about 12% Na2O by mass, 13% CaO by mass, and 75% SiO2 by mass. How much of each reactant would you start with to prepare 0.35 kg of glass?
1562
views